Periodic Trends Models of the Atom Orbitals Electron Configuration Valence Electrons 10 20 30 40 50 40 30 20 10 50 40 30 20 10 50 40 30 20 10 50 40 30.

Slides:

Advertisements

Similar presentations

Periodic Trends. Atomic Radius Atomic Radius (size) is the distance between the nucleus and the outer electrons in an atom.

Advertisements

Periodic Table Trends. Ionization Energy Increasing or Decreasing?

Aim: What are the Properties of Groups and how does the atomic radius change across a period and down a group ? DO Now: 1. Write down the electron configuration.

Which Element? Is highest in electronegativity?. Which Element? Is lowest in electronegativity?

Objectives SWBAT distinguish among the Aufbau principle, the Pauli exclusion principle, and Hund’s rule. SWBAT write electron configurations for selected.

Fall 2011 – Week 8 (Electrons)

Valence Electrons and Electron Configuration Explaining the arrangement of electrons 08/26 to 08/28.

Electron Configurations,

The Periodic Table & Formation of Ions

2.3 Atomic Theories. Greeks (5 th Century B.C.) – coined the term “atoms” to describe invisible particles of which substances were composed Aristotle.

Unit 2 Practice Review Ch. 3,4,5 no periodic trends

In the mid 1800s Demitri Mendeleev worked with 70 elements (only 70 were known at the time). He created the first Periodic Table by arranging the elements.

Organization of the Periodic Table.  Columns of the periodic table  Atoms of elements in the same group have the same # of valence electrons and therefore.

 In general, as we go across a period from left to right, the first ionization energy increases.  Why?  Electrons added in the same principal quantum.

Atoms and the Periodic Table. Atomic Models  Democritus (4 th century B.C.) thought all matter was made of particles he called the atom  Theory was.

Unit 2 Extra Practice October 15 (ODD) October 16 (EVEN)

Anything in black letters = write it in your notes (‘knowts’)

Timberlake LecturePLUS 2000 Characteristics of Atoms Atoms are composed of protons, neutrons, and electrons. Protons and neutrons are located in the nucleus.

Electron Configuration Topic #8 September How was the Atomic Model developed?

Section 11.4 Electron Configurations and Atomic Properties 1.To understand how the principal energy levels fill with electrons in atoms beyond hydrogen.

Bohr Model of the Atom  Bohr’s Atomic Model of Hydrogen  Bohr - electrons exist in energy levels AND defined orbits around the nucleus.  Each orbit.

Atoms and the Periodic Table. Atoms  Atoms are the smallest pieces of matter that contain all the properties of a specific element  Each element contains.

Periodic Law Review Chapter 5. This man organized the periodic table by increasing atomic mass. This man organized the periodic table by increasing atomic.

Chapter 6 Review.

The Periodic Law. Dmitri Mendeleev - discovered that when placed in order of their atomic mass, elements show a repeating pattern of properties. Atomic.

 Knowing the position of electrons helps us with many topics:  Why chemical reactions occur  Why some atoms are more stable than others  Why some.

Electrons, Atoms, and the Periodic Table. ATOM Smallest particle of an element that retains its identity in a chemical reaction VERY SMALL!!! – A pure.

Chapter 3 Atoms and Elements 3.7 Electron Energy Levels 1.

BINGO  Use study guide, worksheets, even questions at end of chapters 5 and 6.  Answer should be an “element”.  Clues may include a list of elements.

Miscellaneous Families Trends Electron Configuration Valence Electrons

Chapter 3 Atoms and Elements 3.7 Electron Energy Levels 1.

Quantum Mechanics. Electron Density Gives the probability that an electron will be found in a particular region of an atom Regions of high electron density.

 What is the electron configuration for Magnesium? What block, group and period does it belong to?  What is the noble gas configuration for Iodine? Is.

Chapter 3Atoms and Elements 3.6 Isotopes and Atomic Mass 1  24 Mg 25 Mg 26 Mg Copyright © 2009 by Pearson Education, Inc.

Chapter 5 The Periodic Law

Review Test Monday April 13 th MC (10 marks) Short answer (37 marks)

Electron Arrangement Review Unit 3. NC Essential Standards Chm Analyze diagrams related to the Bohr model of the hydrogen atom in terms of allowed,

Atoms and the Periodic Table. Atomic Models  Democritus (4 th century B.C.) first theorized that matter was made of particles he called the atom.

Periodic Table And the Periodic Law. Dmitri Mendeleev Russian chemist Created a table by arranging elements according to atomic masses Noticed that chemical.

Quantum Mechanics. Electron Density Gives the probability that an electron will be found in a particular region of an atom Regions of high electron density.

1 st Ionization Energy The amount of energy required to remove an electron from an atom. Trend: Increases left to right across a row. Increases bottom.

Copyright © by Holt, Rinehart and Winston. All rights reserved. ResourcesChapter menu.

SOL Review 2 Atomic Structure And The Periodic Table.

Today’s Do Now 9/11/2014 You will need 4 different colors of writing utensils today – please take these out and have them on your desk 1. Which of the.

ELECTRON CONFIGURATION Agenda Electron Configuration (O/S) HW: Complete Questions on the Handouts.

Periodic Trends. Group Trends Group one, Alkali metals Group two, Alkaline earth metals Groups 3-12, Transition metals Group 17, Halogens Group 18, Noble.

Chapter 5: Electrons in Atoms The chemical properties of atoms, ions, and molecules are related to the arrangement of the electrons within them.

Theories of the Atom. Ernest Rutherford (Gold Foil Experiment) Discovered that atoms have a positively charged central mass called the nucleus Hypothesis:

ELECTRON CONFIGURATION Why are ions more stable than some neutral atoms?

1 Periodic Table II Periodic table arranged according to electron arrangement Periodic table also arranged according to properties? Properties must depend.

Atoms and the Periodic Table. Atoms  Atoms are the smallest pieces of matter that contain all the properties of a specific element  Each element contains.

Atomic Structure. It used to be thought that atoms were small indivisible particles. It was thought that the only difference between the atoms of one.

Periodic Table Atomic Theory Atomic Structure Periodic.

Create an orbital diagram for: Nitrogen Neon

Electron Configuration

Warm-up You will need a periodic table today!!

Progression of Atomic Models

Atomic Mass = All the Isotopes

Chemistry Unit Three Atomic Structure.

Ions, Electrons and Periodicity

Write the Complete Electron Configuration for:

Periodic Trends.

“Test Review” Go through these to practice for your test on Tuesday (answers are on following slides):

OR Why we call it the PERIODIC table

Atomic Structure.

The Atom Grade 9 Science Ms. Raper..

Atoms & the Periodic Table

Valence Electrons.

Electron Configuration

Electronic Configurations

Presentation transcript:

Periodic Trends Models of the Atom Orbitals Electron Configuration Valence Electrons

Topic 1 – 10 Points QUESTION: The first atomic theory, developed by John Dalton, used what model to describe atoms? ANSWER: (tiny solid spheres)

Topic 1 – 20 Points QUESTION: What did J.J. Thompson discover? ANSWER: (the electron)

Topic 1 – 30 Points QUESTION: What two things did Ernest Rutherford’s gold foil experiment discover about the atom? ANSWER: (the nucleus and that the atom is mostly empty space)

Topic 1 – 40 Points QUESTION: How did the atomic model developed by Niels Bohr differ from the model developed a few years earlier by Ernest Rutherford ANSWER: (In the Bohr model, electrons orbit the nucleus at discrete, different energy levels, similar to planets orbiting a sun)

Topic 1 – 50 Points QUESTION: In the quantum model of the atom, we describe electrons as being located in __________ surrounding the nucleus. ANSWER: (orbitals or electron clouds)

Topic 2 – 10 Points QUESTION: What principal energy level and sublevel is lowest in energy and closest to the nucleus? ANSWER: (1s)

Topic 2 – 20 Points QUESTION: How many electrons can you put in an orbital? ANSWER: (2)

Topic 2 – 30 Points QUESTION: The sublevel letters (s,p,d,f) give information about the ________ of the electron cloud. ANSWER: (shape)

Topic 2 – 40 Points QUESTION: How many orbitals are in the “p” sublevel? ANSWER: (3)

Topic 2 – 50 Points QUESTION: Look at the orbital diagram below. What is wrong with it? A. 4s should come before 3p in energy order B. The arrows are not placed in the orbitals according to Hund’s rule C. There should only be an s sublevel in the second energy level D. Nothing is wrong with it ANSWER:B

Topic 3 – 10 Points QUESTION: Write the electron configuration for Lithium ANSWER: (1s 2 2s 1 )

Topic 3 – 20 Points QUESTION: Draw the orbital diagram for Sulfur ANSWER: ()

Topic 3 – 30 Points QUESTION: Write the electron configuration for Argon. ANSWER: (1s 2 2s 2 2p 6 3s 2 3p 6 )

Topic 3 – 40 Points QUESTION: Magnesium has a configuration of 1s 2 2s 2 2p 6 3s 2. What is the configuration of Mg 2+ ? ANSWER: (1s 2 2s 2 2p 6 )

Topic 3 – 50 Points QUESTION: Write the noble gas configuration for Sn (Tin). ANSWER: ()

Topic 4 – 10 Points QUESTION: How many valence electrons does Oxygen have? ANSWER: (6)

Topic 4 – 20 Points QUESTION: Write the valence configuration for Chlorine ANSWER: (3s 2 sp 5 )

Topic 4 – 30 Points QUESTION: Write the valence configuration for Na (sodium). ANSWER: (3s 1 )

Topic 4 – 40 Points QUESTION: What alkaline earth ion has the same valence configuration as Argon? ANSWER: (Ca 2+ )

Topic 4 – 50 Points QUESTION: What is the valence shell configuration of all the noble gases? ANSWER: (s 2 p 6 )

Topic 5 – 10 Points QUESTION: Does atomic radius increase or decrease as you move from left to right across a period in the periodic table? ANSWER: (decreases)

Topic 5 – 20 Points QUESTION: Which element has a higher first ionization energy: Ar, Kr, or Ne ANSWER: (Ne. The electrons are closest to the nucleus in neon, and therefore harder to remove)

Topic 5 – 30 Points QUESTION: Which element is most electronegative, Cesium or Fluorine? ANSWER: (Fluorine)

Topic 5 – 40 Points QUESTION: Arrange the following atoms in order from smallest ionization energy to largest ionization energy: Cl, Si, P, Ar ANSWER: (Si, P, Cl, Ar)

Topic 5 – 50 Points QUESTION: Which of the following atoms would you expect to have the largest atomic radius: A.I B.K C.Ca D.Rb ANSWER: (Rb)